Page 1 of 4
Chapter Review
Key Terms
binary compound (4.1)
binary ionic compound (4.1)
polyatomic ion (4.4)
oxyanion (4.4)
acid (4.5)
Summary
1. Binary compounds can be named systematically by following a set of relatively simple rules. For compounds
containing both a metal and a nonmetal, the metal is
always named first, followed by a name derived from
the root name for the nonmetal. For compounds containing a metal that can form more than one cation
(Type II), we use a Roman numeral to specify the
cation’s charge. In binary compounds containing only
nonmetals (Type III), prefixes are used to specify the
numbers of atoms.
2. Polyatomic ions are charged entities composed of several atoms bound together. They have special names
that must be memorized. Naming ionic compounds
that contain polyatomic ions is very similar to naming
binary ionic compounds.
3. The names of acids (molecules with one or more H
ions attached to an anion) depend on whether the anion contains oxygen.
Questions and Problems
7. Identify each case in which the name is incorrect. Give
the correct name.
a. BaH2, barium hydroxide
b. Na2O, disodium oxide
c. SnCl4, tin(IV) chloride
d. SiO2, silver dioxide
e. FeBr3, iron(III) bromide
8. Write the name of each of the following ionic substances, using the system that includes a Roman numeral to specify the charge of the cation.
a. FeI3
c. HgO
e. CuO
b. MnCl2
d. Cu2O
f. SnBr4
9. Write the name of each of the following ionic substances, using -ous or -ic endings to indicate the charge
of the cation.
a. CoCl2
c. PbO
e. Fe2O3
b. CrBr3
d. SnO2
f. FeCl3
4.2 Naming Binary Compounds That
Contain Only Nonmetals (Type III)
Questions
10. Name each of the following binary compounds of
nonmetallic elements.
a. IF5
c. SeO
e. NI3
b. AsCl3
d. XeF4
f. B2O3
11. Write the name for each of the following binary compounds of nonmetallic elements.
a. GeH4
c. P2S5
e. NH3
b. N2Br4
d. SeO2
f. SiO2
All exercises with blue numbers have answers in the
back of this book.
4.3 Naming Binary Compounds:
A Review
4.1 Naming Compounds That Contain a
Metal and a Nonmetal
Questions
Questions
1. What is a binary compound? Give three examples of
binary compounds.
2. What are the two major types of binary compounds?
3. In an ionic compound, the positive ion is called the
and the negative ion is called the
.
4. In naming ionic compounds, we always name the
first.
5. Although we write the formula of sodium chloride as
NaCl, we realize that NaCl is an ionic compound and
contains no molecules. Explain.
6. Give the name of each of the following simple binary
ionic compounds.
a. NaI
d. CaBr2
g. CsI
b. CaF2
e. SrO
h. Li2O
c. Al2S3
f. AgCl
108
Chapter 4 Nomenclature
12. Name each of the following binary compounds, using the periodic table to determine whether the compound is likely to be ionic (containing a metal and a
nonmetal) or nonionic (containing only nonmetals).
a. B2H6
c. CBr4
e. CuCl2
b. Ca3N2
d. Ag2S
f. ClF
13. Name each of the following binary compounds, using the periodic table to determine whether the compound is likely to be ionic (containing a metal and a
nonmetal) or nonionic (containing only nonmetals).
a. RaCl2
c. PCl3
e. MnF2
b. SeCl2
d. Na3P
f. ZnO
4.4 Naming Compounds That Contain
Polyatomic Ions
Questions
14. What is an oxyanion? How is a series of oxyanions
named? (Give an example.)
Page 2 of 4
15. Which oxyanion of chlorine contains the most oxygen atoms: hypochlorite, chlorite, or perchlorate?
16. Complete the following list by filling in the missing
names or formulas of the indicated oxyanions.
BrO
iodate
IO4
hypoiodite
17. Write the formula for each of the following nitrogencontaining polyatomic ions, including the overall
charge of the ion.
a. nitrate
c. ammonium
b. nitrite
d. cyanide
18. Write the formula for each of the following chlorinecontaining ions, including the overall charge of the ion.
a. chloride
c. chlorate
b. hypochlorite
d. perchlorate
19. Write the formulas of the compounds below (see your
answers to problem 18).
a. magnesium chloride
b. calcium hypochlorite
c. potassium chlorate
d. barium perchlorate
20. Give the name of each of the following polyatomic
anions.
a. MnO4
d. Cr2O72
2
b. O2
e. NO3
2
c. CrO4
f. SO32
21. Name each of the following compounds, which contain polyatomic ions.
a. Fe(NO3)3
d. Al2(SO4)3
b. Co3(PO4)2
e. Cr(C2H3O2)2
c. Cr(CN)3
f. (NH4)2SO3
4.5 Naming Acids
Questions
22. Give a simple definition of an acid.
23. Many acids contain the element
tion to hydrogen.
in addi-
24. Name each of the following acids.
a. HCl
d. HI
g. HBr
b. H2SO4
e. HNO2
h. HF
c. HNO3
f. HClO3
i. HC2H3O2
4.6 Writing Formulas from Names
Problems
25. Write formulas for each of the following simple binary ionic compounds.
a. lithium oxide
b. aluminum iodide
c. silver oxide
d. potassium nitride
e. calcium phosphide
f. magnesium fluoride
g. sodium sulfide
h. barium hydride
26. Write the formula for each of the following binary
compounds of nonmetallic elements.
a. carbon dioxide
b. sulfur dioxide
c. dinitrogen tetrachloride
d. carbon tetraiodide
e. phosphorus pentafluoride
f. diphosphorus pentoxide
27. Write the formula for each of the following compounds that contain polyatomic ions. Be sure to enclose the polyatomic ion in parentheses if more than
one such ion is needed.
a. calcium phosphate
b. ammonium nitrate
c. aluminum hydrogen sulfate
d. barium sulfate
e. ferric nitrate
f. copper(I) hydroxide
28. Write the formula for each of the following acids.
a. hydrocyanic acid
e. hypochlorous acid
b. nitric acid
f. hydrobromic acid
c. sulfuric acid
g. bromous acid
d. phosphoric acid
h. hydrofluoric acid
29. Write the formula for each of the following substances.
a. lithium chloride
b. cuprous carbonate
c. hydrobromic acid
d. calcium nitrate
e. sodium perchlorate
f. aluminum hydroxide
g. barium hydrogen carbonate
h. iron(II) sulfate
i. diboron hexachloride
j. phosphorus pentabromide
k. potassium sulfite
l. barium acetate
Critical Thinking
30. Before an electrocardiogram (ECG) is recorded for a
cardiac patient, the ECG leads are usually coated with
a moist paste containing sodium chloride. What property of an ionic substance such as NaCl is being made
use of here?
31. What is a binary compound? What is a polyatomic anion? What is an oxyanion?
32. Name the following compounds.
a. AuBr3
e. NH3
b. Co(CN)3
f. Ag2SO4
c. MgHPO4
g. Be(OH)2
d. B2H6
Chapter Review
109
Page 3 of 4
33. Name the following compounds.
a. (NH4)2CO3
e. MnO2
b. NH4HCO3
f. HIO3
c. Ca3(PO4)2
g. KH
d. H2SO3
charges of 1, 2, and 3, respectively. Consider also
the nonmetallic elements D, E, and F, which form anions that have charges of 1, 2, and 3, respectively. Write the formulas of all possible compounds
between metal M and nonmetals D, E, and F.
34. Most metallic elements form oxides, and often the oxide is the most common compound of the element
that is found in the earth’s crust. Write the formulas
for the oxides of the following metallic elements.
a. potassium
e. zinc
b. magnesium
f. lead(II)
c. iron(II)
g. aluminum
d. iron(III)
35. Consider the hypothetical metallic element M, which
is capable of forming stable simple cations that have
36. Complete Table 4.A (below) by writing the names and
formulas for the ionic compounds formed when the
cations listed across the top combine with the anions
shown in the left-hand column.
37. Complete Table 4.B (below) by writing the formulas
for the ionic compounds formed when the anions
listed across the top combine with the cations shown
in the left-hand column.
38. For each of the negative ions listed in column 1, use
the periodic table to find in column 2 the total num-
TABLE 4.A
Ions
Fe2
Al3
Na
Ca2
NH4
Fe3
Ni2
Hg22 Hg2
CO32
BrO3
C2H3O2
OH
HCO3
PO43
SO32
ClO4
SO42
O2
Cl
TABLE 4.B
Ions
calcium
strontium
ammonium
aluminum
iron(III)
nickel(II)
silver(I)
gold(III)
potassium
mercury(II)
barium
nitrate
sulfate
hydrogen
sulfate
dihydrogen
phosphate
oxide
chloride
Page 4 of 4
ber of electrons the ion contains. A given answer may
be used more than once.
Column 1
[1]
[2]
[3]
[4]
[5]
[6]
[7]
[8]
[9]
[10]
2
Se
S2
P3
O2
N3
I
F
Cl
Br
At
Column 2
[a]
[b]
[c]
[d]
[e]
[f]
[g]
[h]
[i]
[j]
18
35
52
34
36
54
10
9
53
86
39. For each of the following processes that show the formation of ions, complete the process by indicating
the number of electrons that must be gained or lost
to form the ion. Indicate the total number of electrons in the ion, and in the atom from which it was
made.
a. Al n Al3
d. F n F
2
b. S n S
e. Zn n Zn2
c. Cu n Cu
f. P n P3
40. For each of the following atomic numbers, use the periodic table to write the formula (including the charge)
for the simple ion that the element is most likely to
form.
a. 36
d. 81
b. 31
e. 35
c. 52
f. 87
41. For the following pairs of ions, use the principle of
electrical neutrality to predict the formula of the binary compound that the ions are most likely to form.
a. Na and S2
e. Cu2 and Br
b. K and Cl
f. Al3 and I
2
2
c. Ba and O
g. Al3 and O2
2
2
d. Mg and Se
h. Ca2 and N3
42. Give the name of each of the following simple binary
ionic compounds.
a. BeO
e. HCl
b. MgI2
f. LiF
c. Na2S
g. Ag2S
d. Al2O3
h. CaH2
43. In which of the following pairs is the name incorrect?
a. SiI4, silver iodide
b. CoCl2, copper(II) chloride
c. CaH2, hydrocalcinic acid
d. Zn(C2H3O2)2, zinc acetate
e. PH3, phosphoric trihydride
44. Write the name of each of the following ionic substances, using the system that includes a Roman numeral to specify the charge of the cation.
a. FeBr2
d. SnO2
b. CoS
e. Hg2Cl2
c. Co2S3
f. HgCl2
45. Name each of the following binary compounds.
a. XeF6
d. N2O4
b. OF2
e. Cl2O
c. AsI3
f. SF6
46. Name each of the following compounds.
a. Fe(C2H3O2)3
d. SiBr4
b. BrF
e. Cu(MnO4)2
c. K2O2
f. CaCrO4
47. Name each of the following compounds, which contain polyatomic ions.
a. LiH2PO4
d. Na2HPO4
b. Cu(CN)2
e. NaClO2
c. Pb(NO3)2
f. Co2(SO4)3
48. Write the formula for each of the following simple binary ionic compounds.
a. calcium chloride
b. silver(I) oxide (usually called silver oxide)
c. aluminum sulfide
d. beryllium bromide
e. hydrosulfuric acid
f. potassium hydride
g. magnesium iodide
h. cesium fluoride
49. Write the formula for each of the following binary
compounds of nonmetallic elements.
a. sulfur dioxide
b. dinitrogen monoxide
c. xenon tetrafluoride
d. tetraphosphorus decoxide
e. phosphorus pentachloride
f. sulfur hexafluoride
g. nitrogen dioxide
50. Write the formula of each of the following ionic substances.
a. sodium dihydrogen phosphate
b. lithium perchlorate
c. copper(II) hydrogen carbonate
d. potassium acetate
e. barium peroxide
f. cesium sulfite
51. Write the formula for each of the following compounds, which contain polyatomic ions. Be sure to
enclose the polyatomic ion in parentheses if more
than one such ion is needed to balance the oppositely
charged ion(s).
a. silver(I) perchlorate (usually called silver perchlorate)
b. cobalt(III) hydroxide
c. sodium hypochlorite
d. potassium dichromate
e. ammonium nitrite
f. ferric hydroxide
g. ammonium hydrogen carbonate
h. potassium perbromate
Chapter Review
111